The concentration of sodium sulphate in the resultant solution after neutralizing 20.0 mL of 1.00M sulphuric acid with 2.00M sodium hydroxide is 0.500 mol/L. This conclusion is based on the stoichiometry of the neutralization reaction, where one mole of sulphuric acid reacts with two moles of sodium hydroxide to produce one mole of sodium sulphate. The calculation confirms that the final concentration of sodium sulphate is accurate, assuming complete neutralization.
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Probably not correct, but you haven't included your working so it's not possible to see where we disagree.DavidQT said:3. In an experiment, 2.00M sodium hydroxide solution was added to 20.0mL of 1.00M sulphuric acid until the acid was just completely neutralized. What is the concentration of sodium sulphate in the resultant solution?
My final answer is 0.500mol/l. Am i correct.